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dangina [55]
3 years ago
11

How does fire impact the various populations of trees?

Chemistry
1 answer:
Anuta_ua [19.1K]3 years ago
5 0

It plays a key role in shaping ecosystems by serving as an agent of renewal and change. But fire can be deadly, destroying homes, wildlife habitat and timber, and polluting the air with emissions harmful to human health. Fire also releases carbon dioxide a key greenhouse gas into the atmosphere

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Which of these is a biotic factor in a Forest
Kryger [21]
Plants, animals and bacteria
5 0
2 years ago
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Please help!
cluponka [151]
IT IS D FOCAL POINT
P.S. im in middle school not trying to brag

3 0
3 years ago
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You need 1.2 moles of H2SO4 for an experiment. You weigh out 100g of this colorless syrupy liquid. Do you have enough?
Sladkaya [172]
Answer is: not enough <span>colorless syrupy liquid.
</span>n(H₂SO₄) = 1,2 mol.
M(H₂SO₄) = 2Ar(H) + Ar(S) + 4Ar(O) · g/mol.
M(H₂SO₄) = 2·1 + 32 + 4·16 · g/mol.
M(H₂SO₄) = 98 g/mol.
m(H₂SO₄) = n(H₂SO₄) · M(H₂SO₄).
m(H₂SO₄) = 1,2 mol · 98 g/mol.
m(H₂SO₄) = 117,6 g needed.
100 g is less that 117,6 g.
8 0
3 years ago
a compound has an empirical formula of CH2 what is the molecular formula if it's molar mass is 252.5 grams/mol
Goryan [66]

Empirical formula is the simplest ratio of components making up the compound. the molecular formula is the actual ratio of components making up the compound.

the empirical formula is CH₂. We can find the mass of CH₂ one empirical unit and have to then find the number of empirical units in the molecular formula.

Mass of one empirical unit - CH₂ - 12 g/mol x 1 + 1 g/mol x 2 = 12 = 14 g

Molar mass of the compound is - 252 .5 g/mol

number of empirical units = molar mass / mass of empirical unit

                                           = \frac{252.5 g/mol}{14 g}

                                           = 18 units

Therefore molecular formula is - 18 times the empirical formula

molecular formula  - CH₂ x 18 = C₁₈H₃₆                                            

molecular formula is C₁₈H₃₆  

8 0
3 years ago
A smaple of 1cm cuvette gives an absorbance reading of 0.558. if they absorptivity for this sample is 15000l/(mol.cm), what is t
Mazyrski [523]
To solve this problem, we use Beer's Law: A= ε.l.c
A is the absorbance- 0,558
<span>ε is</span> the molar absorptivity- is <span>15000 </span><span><span>L⋅mol-1</span><span>cm-1</span></span>
<span>l is </span>the length of the cuvette- 1 cm
<span>c is</span> the molar concentration

Applying the formula,
0,558= 15000 x 1 x c
0,558/15000= c
c= <span>3.72×<span>10⁻⁵ </span> <span>mol⋅L<span>⁻¹</span></span></span>
<span />
3 0
3 years ago
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